Final answer:
The half-life for the given zero-order reaction, with an initial concentration of A as 2 M and a rate of 2 M/s, is 1 second because the concentration of A decreases by 1 M each second regardless of its current value.
Step-by-step explanation:
The student is asking about the half-life of a zero-order reaction, where the chemical equation is A→B+C. The initial concentration of reactant A is 2 M, and the rate of reaction is given as 2 M/s. The half-life of a zero-order reaction is the time it takes for the reactant concentration to decrease to half its initial value.
In a zero-order reaction, the rate of reaction is independent of the concentration of reactants. The rate of consumption of A is constant. To find the half-life, we can set up the zero-order kinetics equation:
Rate = k[A]°, where k is the rate constant. Given that the rate is 2 M/s, and the reaction starts at 2 M, it would take 1 second for the concentration of A to drop to 1 M, which is half of its initial concentration. Therefore, the half-life of this reaction is 1 second.
It's important to note that the provided information about second-order reactions is not applicable to this specific zero-order reaction scenario.